[Foobarz]

 If this NH4Cl solution is assumed to be ideal and is completely dissociated into ions, calculate the vapor pressure of this solution at 29.0 °C. (the molality of the solution from the previous question is 4.76 m)

Ok, so looking at the answer, the problem makes no sense at all. It goes into Raoult's law, which I understand. Raoult's law needs to know the vapor pressure of the pure solvent. The question (in the answer) just gives out the vapor pressure of water as 29.8 mmHg. But still, how in the world am I supposed to figure out the vapor pressure of water at 29 C using just the information provided? Or was it in an error? Yet this is an old 1976 B AP Chemistry Free Response question. . .

[UG]

Perhaps you need to use the Clausius-Clapeyron equation

[Foobarz]

OH MY THAT Is going to be a tedious task. . .

[Foobarz]

Darn it the vapor pressure I got was 34.5 mmHg. That's not what the explanation uses; it uses 29.8 mmHg. I still don't get how that was received. Could anyone help me?

http://sentinelchem.wikispaces.com/file/view/Properties+of+Solutions+notes.pdf
It's on this website. Search for 1976 B.

[UG]

Would you mind showing us your working and what data you used?

[Foobarz]

Well, dont know how to type it out so here. . .

[UG]

Hmmm... that seems weird. I used the saturated vapour pressure of water at 25^oC (23.8 mmHg) and got an answer around 29.6 mmHg

[Foobarz]

Yes, that is quite odd. . .
Water does boil at 760 mmHg right?

[Foobarz]

AHHH I'm so ANGRY WHAT DID I DO WRONG??|
It makes no sense. . .